Correct Answer: Option B

Explanation

The oxidation state of nitrogen in N\(_2\)O\(_3\) is +3. This is calculated using the rule that oxygen typically has an oxidation state of -2 in compounds, and the sum of all oxidation states in a neutral compound is zero. 

In N\(_2\)O\(_5\): N\(_2\)O\(_5\) = 0 

               2(N) + ( -2 x 5) = 0

             2N - 10 = 0

              N = \(\frac{10}{2}\) = +5

In N\(_2\)O\(_3\): N\(_2\)O\(_3\) = 0 

               2(N) + ( -2 x 3) = 0

             2N - 6 = 0

              N = \(\frac{6}{2}\) = +3

In N\(_2\)O\(_4\): N\(_2\)O\(_4\) = 0 

               2(N) + ( -2 x 4) = 0

             2N - 8 = 0

              N = \(\frac{8}{2}\) = +4

In N\(_2\)O: N\(_2\)O = 0 

               2(N) + (-2) = 0

             2N - 2 = 0

              N = \(\frac{2}{2}\) = +1

The correct option is B - N\(_2\)O\(_3\).

There is an explanation video available below.

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